Ion-solvent interaction and the viscosity of strong-electrolyte solutions

Abstract

It is shown that there is a relationship between the temperature dependence of the viscosity of aqueous solutions and the ion-solvent interaction. For the temperature range 1542.5" C and for different charge types, the B-coefficient in Jones and Dole's equation can be split into contributions (B&) due to the separate ions. Two rules are proposed for the dependence of Bion values on the nature of the ions and on the temperature. It is shown that the Bion values, the apparent molal heat capacities (C,o) and apparent molal volumes ($0) of single ions show an almost identical temperature dependence.* Since the B-values used by Wolfenden and Cox were in several cases subject to an uncertainty of cu. 15 %, the exact additivity could not be regarded as established.

Dielectric Relaxation of Aqueous Solution with Low-molecular-weight Nonelectrolytes and Its Relationship with Solution Structure

“…The parameter IX was proved to be correlated well with aqueous solution structure parameters reported in the literature: Bcoefficient of viscosity for electrolytes, 13) hydration parameter for nonelectrolytes,14) and number of equatorial-OH for saccharides. 1, urea; 2, formamide; 3. tert-butyl alcohol; 4, ethanol; 5, 2-propanol; 6, ribose; 7.…”

The Viscosity and Conductivity of Aqueous Solutions of Electrolytes Mixed with Glycine and Urea

“…Some studies of the electrochemical properties of aqueous solutions of strong electrolytes using several methods have been reported, [1][2][3][4] but only a few data are available in the literature5-8) for aqueous solutions of mixed electrolytes. The purpose of the present study is to obtain some information concerning hydration and related problems, and to determine the behavior of weak electrolytes from measurements of the viscosity, density and conductivity of various electrolyte solutions in which weak electrolytes are mixed with strong electrolytes.…”

Measurement of Limiting Partition Coefficient in Progressive Freeze-Concentration

“…The interfacial water molecules adjacent to Na ϩ are less mobile and their entropy is lower than those adjacent to K ϩ (Collins & Washabaugh, 1985). The viscosity of NaCl solution is higher than KCl solution at the same molar concentration (Kaminsky, 1957). These differences correspond to the difference in the solution structure between the two solutions, and this difference in structure might have affected the difference in K 0 observed in the present case.…”

“…The hydration state of Na ϩ is much stronger than K ϩ , which affects the aqueous solution structure through the hydrogen bonding. Na ϩ is so-called "water-structure-forming" while K ϩ is "water-structure-breaking" (Kaminsky, 1957;Herscovits & Kelly, 1973). The interfacial water molecules adjacent to Na ϩ are less mobile and their entropy is lower than those adjacent to K ϩ (Collins & Washabaugh, 1985).…”